Download AP Semestar Exam REVIEW

AP Semestar Exam
Section I: Multiple Choice
60 minutes
You may not have access to a calculator during this section
Identify the choice that best completes the statement or answers the question.
____
1. Which method is best for separating a mixture of ethyl alcohol and water?
a. distillation
b. light absorption
c. electrolysis
d. gas-liquid chromatography
e. filtration
____
2. All of the following relationships are true EXCEPT
a. 0.328 g = 328 mg.
b. 23 km < 4.5 107 mm.
c. 0.84 kg > 8.4 104 mg.
d. 41.3 mL > 8.72 10-2 L.
e. 1.3 nm = 1.3 10-6 mm.
____
3. All of the following statements are true EXCEPT
a. a proton carries a +1 charge and an electron carries a -1 charge.
b. the nucleus of an atom has a negative charge.
c. an alpha particle is a helium atom minus its electrons.
d. a neutron is an uncharged particle with a mass slightly greater than a proton.
e. more than 99.9% of an atom's mass is concentrated in the nucleus.
____
4. Rank the subatomic particles from least to greatest mass.
a. electrons = neutrons = protons
b. electrons = protons < neutrons
c. electrons < neutrons = protons
d. electrons < protons < neutrons
e. electrons < neutrons < protons
____
5. All atoms of the same element have the same number of __________ .
a. neutrons
b. protons
c. protons and neutrons
d. electrons and neutrons
e. protons, neutrons, and electrons
____
6. What is the identity of
a. zinc
b. silver
c. iridium
d. cesium
e. manganese
____
7. Identify the ions and their charges in KH2PO4.
a. K+, H+, P3-, O2-
?
b.
c.
d.
e.
K+, H2+, P3-, O8K+, H22+, P-1, O4-2
K+, H2PO4K+, H2+, PO43-
____
8. What is the correct name for K3PO4?
a. tripotassium phosphate
b. potassium(I) monophosphorus tetraoxide
c. potassium(I) phosphate
d. potassium phosphate
e. potassium phosphide
____
9. What is the correct formula for potassium dichromate?
a. K2Cr2O7
b. K2(Cr2O7)2
c. K2CrO4
d. K2(CrO4)2
e. KCrO4
____ 10. What is the correct name for HI(aq)?
a. hydroiodic acid
b. hydrogen iodide ion
c. monohydrogen monoiodide
d. iodate acid
e. iodine hydride
____ 11. Which of the following samples contains the largest number of atoms?
a. 2.0 moles of H3PO4
b. 3.0 moles of H2SO3
c. 4.0 moles of HNO3
d. 6.0 moles of HClO
e. 8.0 moles of HBr
____ 12. What mass of oxygen is present in 10.0 grams of potassium nitrate (KNO3)?
a. 4.75 g
b. 5.43 g
c. 6.39 g
d. 8.00 g
e. 9.17 g
____ 13. What is the maximum volume of 0.25 M KCl(aq) that can be prepared from 75 g KCl(s)?
a. 0.33 L
b. 1.0 L
c. 3.0 L
d. 4.0 L
e. 19 L
____ 14. Which of the following methods correctly describes the preparation of 1.00 L of an aqueous solution of 0.500
M NaOH?
a. Place 0.500 g NaOH(s) in a flask and dilute to 1.00 L with water.
b. Place 0.500 g NaOH(s) in a flask and add 1.00 L of water.
c. Place 20.0 g NaOH(s) in a flask and dilute to 1.00 L with water.
d. Place 20.0 g NaOH(s) in a flask and add 1.00 L of water.
e. Place 40.0 g NaOH(s) in a flask and add 500 g of water.
____ 15. Precipitation reactions occur
a. when group 1 cations are mixed with group 17 anions.
b. when insoluble reactants are mixed.
c. when ionic compounds react to form non-ionic products.
d. predominantly with halide salts.
e. when soluble ionic reactants combine to form insoluble products.
____ 16. If aqueous solutions of sodium sulfate and barium chloride are mixed, a white precipitate forms. What is the
identity of the precipitate?
a. Na2Ba
b. NaCl2
c. NaCl
d. BaSO4
e. Ba2SO4
____ 17. Which of the following ionic compounds are likely to be soluble in water: Mg(OH)2, Pb(NO3)2, AgI, Na2CO3,
and Cu3(PO4)3?
a. Na2CO3 only
b. Pb(NO3)2 and Na2CO3
c. Mg(OH)2, Na2CO3, and Cu3(PO4)3
d. Mg(OH)2, AgI, and Cu3(PO4)3
e. Pb(NO3)2, AgI, Na2CO3, and Cu3(PO4)3
____ 18. What net ionic reaction occurs when aqueous solutions of potassium carbonate and iron(III) bromide are
mixed?
a. CO32-(aq) + 2Fe+(aq)  Fe2(CO3)(s)
b. 3CO32-(aq) + 2Fe3+(aq)  Fe2(CO3)3(s)
c. 3CO32-(aq) + 6Fe+(aq)  3Fe2CO3(s)
d. 3K2CO3(aq) + 2Fe3+(aq) + 6Br-(aq)  Fe2(CO3)3(s) + 6KBr(s)
e. no reaction occurs
____ 19. Write a balanced net ionic equation for the reaction of aluminum hydroxide, Al(OH)3, with nitric acid.
a. Al(OH)3(s) + 3H+(aq)  Al3+(aq) + 3H2O
b. Al(OH)3(s) + 3H+(aq)  AlH3(s) + 3OH-(aq)
c. (OH)3(aq) + 3H+(aq)  3H2O
d. 3OH-(aq) + 3H+(aq)  3H2O
e. Al3+(aq) + 3NO3-(aq)  Al(NO3)3(aq)
____ 20. Identify all of the spectator ions in the reaction below.
Zn(OH)2(s) + 2H+(aq) + 2NO3-(aq)  Zn2+(aq) + 2NO3-(aq) + 2H2O
a.
b.
c.
d.
e.
Zn(OH)2
NO3Zn2+
H+
H+ and NO3-
____ 21. Which list contains only strong acids?
a. HCl, HNO3, HF, HClO4
b.
c.
d.
e.
H2SO4, H3PO4, HClO4, NH3
HCl, HNO3, H3PO4, HClO4
HCl, H2SO4, HClO4, HI
HNO3, H2SO4, NaOH, H3PO4
____ 22. Which of the following are strong bases: NH3, NaOH, Ba(OH)2, and HF?
a. NH3 and HF
b. NaOH and Ba(OH)2
c. NH3 and NaOH
d. NaOH, Ba(OH)2, and HF
e. NH3, NaOH, Ba(OH)2, and HF
____ 23. What is the net ionic equation for the reaction of lithium hydroxide with hydroiodic acid?
a. H+ + I-  HCl(s)
b. Li+ + I-  KCl(s)
c. LiOH(aq) + HI(aq)  LiI(s) + H2O
d. LiOH(s) + H+(aq)  Li+(aq) + H2O
e. OH-(aq) + H+(aq)  H2O
____ 24. When HCl(g) and NH3(g) are mixed, a white solid forms. What is the balanced equation for this reaction?
a. HCl(g) + NH3(g)  NH4Cl(s)
b. HCl(g) + NH3(g)  NH2Cl(g) + H2(s)
c. HCl(g) + NH3(g)  NH4(s) + Cl(g)
d. HCl(g) + NH3(g)  NH2Cl(s) + H2(g)
e. 3HCl(g) + NH3(g)  NCl3(s) + 3H2(g)
____ 25. A reducing agent is a species that
a. takes a proton from an Arrhenius acid.
b. is reduced in a chemical reaction.
c. gains electrons in a chemical reaction.
d. loses electrons in a chemical reaction.
e. gives a proton to an Arrhenius base.
____ 26. Assign oxidation numbers to each atom in calcium perchlorate, Ca(ClO4)2.
a. Ca = 0; Cl = 0; O = 0
b. Ca = 0; Cl = -1; O = -2
c. Ca = +2; Cl = -1; O = -2
d. Ca = +2; Cl = +5; O = -2
e. Ca = +2; Cl = +7; O = -2
____ 27. Identify the oxidizing and reducing agents in the redox reaction below.
3Cu(s) + 8H+(aq) + 2NO3-(aq)  3Cu2+(aq) + 2NO(g) + 4H2O
a.
b.
c.
d.
e.
reducing agent: Cu; oxidizing agent: Cu2+
reducing agent: NO3-; oxidizing agent: NO
reducing agent: Cu; oxidizing agent: NO3reducing agent: NO3-; oxidizing agent: Cu
reducing agent: H+; oxidizing agent: NO
____ 28. What is the oxidation half-reaction for the reaction of zinc with hydrochloric acid?
Zn(s) + 2H+(aq)  Zn2+(aq) + H2(g)
a.
b.
c.
d.
e.
Zn(s)  Zn2+(aq) + 2eZn(s) + 2e-  Zn2+(aq)
2H+(aq)  H2(g) + 2e2H+(aq) + 2e-  H2(g)
none of the above
____ 29. What is the reduction half-reaction for the equation below?
5Fe2+(aq) + MnO4-(aq) + 8H+(aq)  5Fe3+(aq) + Mn2+(aq) + 4H2O
a.
b.
c.
d.
e.
MnO4-(aq) + 5e-  Mn2+(aq) + 2O2(g)
MnO4-(aq) + 8H+(aq) + 5e-  Mn2+(aq) + 4H2O
Fe2+(aq) + e-  Fe3+(aq)
8H+(aq) + 8e-  8H2O
none of the above
____ 30. If the volume of a confined gas is doubled at constant temperature, what change is observed?
a. The pressure of the gas is decreased to
of its original value.
b. The pressure of the gas is decreased to
of its original value.
c. The pressure of the gas is increased to twice its original value.
d. The density of the gas is doubled.
e. The velocities of the molecules are doubled.
____ 31. All of the following relationships are false for gases EXCEPT
a. volume is inversely proportional to the moles of gas.
b. volume is directly proportional to pressure in mm Hg.
c. volume is directly proportional to pressure in atmospheres.
d. volume is directly proportional to temperature in Kelvin.
e. volume is directly proportional to the gas constant R.
____ 32. At what temperature does 1.00 atm of carbon dioxide (CO2) gas have the same density as 1.00 atm of helium
gas at 25ºC?
a. 0 K
b. 25 K
c. 482 K
d. 983 K
e. 3.28 103 K
____ 33. Sulfur burns in oxygen with a deep blue flame to produce sulfur dioxide. If 5.85 g S8 and 1.00 atm of O2
completely react in a 5.00 L flask (at 25ºC), determine the partial pressure of SO2 (at 25ºC) and the total
pressure in the flask.
S8(s) + 8O2(g)  8SO2(g)
a.
b.
c.
d.
e.
O2 = 0 atm, SO2 = 1.00 atm, total pressure = 1.00 atm
O2 = 0.093 atm, SO2 = 0.917 atm, total pressure = 1.00 atm
O2 = 0.107 atm, SO2 = 0.893 atm, total pressure = 1.00 atm
O2 = 0.855 atm, SO2 = 0.145 atm, total pressure = 1.00 atm
O2 = 0.917 atm, SO2 = 0.163 atm, total pressure = 1.08 atm
____ 34. All of the following are properties of gases according to the kinetic theory EXCEPT
a. gases consist of mostly empty space.
b. attractive forces cause gas molecules to collide.
c. gas pressure is caused by collisions of molecules with the container walls.
d. collisions between gas molecules are elastic.
e. gas molecules are in constant motion.
____ 35. At a given temperature, molecules of different gases
a. have the same average kinetic energy of translational motion.
b. have the same average velocity.
c. have the same diameter.
d. have the same density.
e. have identical masses.
____ 36. Which conditions will cause the greatest deviation from the ideal gas law?
a. 100 atm and 500 K
b. 100 atm and 10 K
c. 0.001 atm and 500 K
d. 0.001 and 10 K
e. 0.001 and 273 K
____ 37. One way in which real gases differ from ideal gases is that the molecules of a real gas
a. have no kinetic energy.
b. move in curved paths.
c. have no mass.
d. occupy no volume.
e. are attracted to each other.
____ 38. What is the ground state electron configuration of 25Mn?
a. 1s22s22p63s23p63d64s1
b. 1s22s22p63s23p63d54s2
c. 1s22s22p63s23p63d7
d. 1s22s22p63s23p63d5
e. 1s22s22p63s23p64s24d5
____ 39. What is the electron configuration of Cu+?
a. [Ar]3d8
b. [Ar]3d9
c. [Ar]3d10
d. [Ar]3d84s2
e. [Ar]3d94s1
____ 40. What is the correct orbital diagram for phosphorus?
a.
b.
c.
d.
1s
2s
2p
()
()
()
()
()
()
()
()
()()()
()()()
()()()
()()()
e. ()
() ()()()
3s
3p
() ()()()
() ()()()
()
()()()
____ 41. In general, ionization energies (What trend?)
a. increase down a group and increase across a period.
b. increase down a group and decrease across a period.
c. decrease down a group and increase across a period.
d. decrease down a group and decrease across a period.
e. increase with atomic mass and increase with atomic radii.
____ 42. Place the following atoms in order of increasing size: Al, Cl, Mg, O, and P.
a. Cl < O < P < Al < Mg
b. Cl < P < Al < Mg < O
c. O < Cl < P < Al < Mg
d. O < Mg < Al < P < Cl
e. none of the above
____ 43. A pair of electrons that is shared between two atoms is
a. a covalent bond.
b. a lone pair.
c. a double bond.
d. an ionic bond.
e. both a covalent bond and a double bond.
____ 44. What is the expected number of valence electrons for an element in group 15?
a. 0
b. 1
c. 3
d. 5
e. 8
____ 45. Which of the following is a correct Lewis structure for oxygen?
a.
b.
c.
d.
e.
____ 46. Which of the following molecules or ions has the same electronic structure as N2?
a. O2
b. CNc. CO
d. Answers a and c are correct.
e. Answers b and c are correct.
____ 47. What is the correct Lewis structure of SF4?
a.
b.
c.
d.
e.
____ 48. Which of the following are correct resonance structures of SO3?
____ 49. Formal charge is
a. the absolute value of the charge on a polyatomic anion or cation.
b. the difference between the number of lone pairs of electrons and shared pairs of electrons
on any atom in a Lewis structure.
c. the difference between the number of valence electrons and the number of protons in any
given atom.
d. equal to the number of valence electrons in a free atom minus the number of shared in
covalent bonds.
e. the difference between the number of valence electrons in a free atom and the number of
electrons assigned to the atom in a Lewis structure.
____ 50. Use VSEPR theory to predict the molecular geometry of IF5.
a. octahedral
b. square planar
c. tetrahedral
d. see-saw
e. square pyramidal
____ 51. What are the bond angles in CO32-?
a. 90º
b. 109.5º
c. 120º
d. 90º and 120º
e. 180º
____ 52. What is the hybridization of the carbon atoms in benzene, C6H6?
a. sp
b. sp2
c. sp3
d. sp3d
e. sp3d2
____ 53. How many sigma and pi bonds are present in the following molecule?
____ 54. All of the following statements are true EXCEPT
a. the value of q is negative in an endothermic process.
b. heat flows from the system into the surroundings in an exothermic process.
c. the value of q is positive when heat flows into a system from the surroundings.
d. enthalpy is a state property.
e. in an endothermic process heat flows from the surroundings into the system.
____ 55. All of the following statements are true EXCEPT
a. the enthalpy change of an endothermic reaction is positive.
b. at constant pressure the heat flow for a reaction equals the change in enthalpy.
c. H for a reaction is equal in magnitude but opposite in sign to H for the reverse reaction.
d. enthalpy is a state function.
e. enthalpy change is dependent upon the number of steps in a reaction.
____ 56. Equilibrium has been established between a liquid and its vapor when
a. there are equal quantities of liquid and vapor.
b. all of the liquid has evaporated.
c. the liquid reaches its boiling point.
d. evaporation ceases and the concentrations of liquid and vapor remain constant.
e. the rate of condensation equals the rate of evaporation.
____ 57. For an ideal gas, a plot of ln P versus 1/T (in Kelvin) yields a straight line with a slope equal to
a. -Hvap.
b. Hvap.
c. -Hvap/R.
d. 1/-Hvap.
e. -Hvap/RT.
____ 58. The normal boiling point of a liquid is
a. 373 K.
b. the temperature at which a liquid's vapor pressure equals 1 atm.
c. the pressure at which the liquid boils at 373 K.
d. dependent upon the volume of the liquid.
e. dependent upon the pressure above the liquid.
____ 59. On the phase diagram below, which point corresponds to conditions where only the gas phase exists?
____ 60. Which of the following pure substances will have hydrogen bonds?
____ 61. Which of the following substances will exhibit dipole forces?
a. SO3
b. H2S
c. CH4
d. SF6
e. N2
____ 62. All of the following statements are correct EXCEPT
a. metals have high electrical conductivity.
b. metals are typically insoluble in water.
c. ionic solids are always soluble in water.
d. ionic solids usually have high melting points.
e. network covalent solids are usually poor electrical conductors.
____ 63. Express the rate of the reaction below in terms of the formation of dinitrogen pentaoxide.
4NO2(g) + O2(g)  2N2O5(g)
____ 64. Which of the statements concerning the relative rates of reaction is correct for the chemical equation below?
N2(g) + 3H2(g)
a.
b.
c.
d.
e.
2NH3(g)
The rate of disappearance of N2 equals 1/4 the rate of formation of NH3.
The rate of disappearance of N2 equals the rate of formation of NH3.
The rate of disappearance of N2 is twice the rate of formation of NH3.
The rate of disappearance of N2 is three times the rate of disappearance of H2.
The rate of disappearance of N2 is 1/3 the rate of disappearance of H2.
____ 65. Dinitrogen pentaoxide decomposes to nitrogen dioxide and oxygen according to the following balanced
chemical equation and rate expression.
2N2O5(g)
4NO2(g) + O2(g)
rate = k[N2O5]
What is the overall reaction order?
____ 66. What are the units of the rate constant for the rate expression for the following chemical equation?
2NO(g) + Cl2(g)  2NOCl(g)
rate = k[NO]2 [Cl2]
____ 67. The reaction rate of CO and NO2 in the reaction
CO(g) + NO2(g)  CO2(g) + NO(g)
is measured using the initial rates method. The results are tabulated below.
[CO] (mol/L)
8.00 10-4
8.00 10-4
1.60 10-3
NO2 (mol/L)
5.50 10-4
11.0 10-3
5.50 10-4
-([CO]/t (mol/L·s)
8.40 10-8
1.68 10-7
1.68 10-7
Determine the rate expression and calculate the rate constant for the reaction.
____ 68. What are the units of the rate constant for a first-order reaction?
____ 69. For the second-order decomposition reaction,
2A  B
rate = k[A]2
which of the following relationships yields a straight line plot?
____ 70. Which equation is used to calculate the half-life of the second-order equation below?
2A  B rate = k[A]2
____ 71. The correct form of the Arrhenius equation is
____ 72. In the Brønsted-Lowry model an acid is
a.
b.
c.
d.
e.
____ 73. Which of the following equilibrium constant expressions represents the ionization of water?
____ 74. What is the correct expression for the calculation of pH?
____ 75. Which of the following mathematical equations corresponds to the acid dissociation constant (Ka)?